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3 years ago

Consider this reaction:

Chemistry

2 answers:

kifflom [539]3 years ago

5 0

Answer:

Lowering the volume of H2 gas

Explanation:

According to Le Chatelier's principle when a reaction is at equilibrium is subject to changes in temperature, pressure and concentration the equilibrium will then shift in a direction to undo the effect of the induced change.

The given reaction is:

$Zn(s) + 2HCl(aq)\rightleftharpoons ZnCl2(aq) + H2(g)$

In order to decrease the rate of production of ZnCl2 the reaction needs to shift to the left. This can be achieved by lowering the volume of H2 gas which would increase its pressure. Based on Le Chatelier's principle, this would shift the equilibrium in a direction that would lower the H2 pressure i.e. to the left thereby also decreasing the production of ZnCl2.

Len [333]3 years ago

3 0

Dilution of hcl because less no of mole of hcl would be reacting to form zncl2

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You are asked to write observations about a 100g sample of Nitrogen-16 before it decays, but you're running late. In order to ma

san4es73 [151]

Answer:

You cannot make observations if you are 57 seconds late into the lab.

Explanation:

The atomic nucleus can split by decay into 2 or more particles as a result of the instability of its atomic nucleus due to the fact that radioactive elements possess an unstable atomic nucleus.

Now, the primary particles which are emitted by radioactive elements in order to make them decay are alpha, beta & gamma particles.

The half life equation is;

N_t = N₀(½)^(t/t_½)

Where:

t = duration of decay

t_½ = half-life

N₀ = number of radioactive atoms initially

N_t = number of radioactive atoms remaining after decay over time t

We are given;

t = 57 secs

N₀ = 100 g

Now, half life of Nitrogen-16 from online sources is 7.2 seconds. t_½ = 7.2

Thus;

N_t = 100(1/2)^(57/7.2)

N_t = 0.4139g

We are told that In order to make observations, you require at least .5g of material.

The value of N_t you got is less than 0.5g, therefore you cannot make observations if you are 57 seconds late.

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3 years ago